English

Complete the Following Statement by Selecting the Correct Alternative from the Choices Given: for a Spontaneous Reaction δG° and E° Cell Will Be Respectively: - Chemistry (Theory)

Advertisements
Advertisements

Question

Complete the following statement by selecting the correct alternative from the choices given:  

For a spontaneous reaction ΔG° and E° cell will be respectively:

Options

  • -ve and +ve

  • +ve and -ve

  • +ve and +ve

  • -ve and -ve

MCQ

Solution

-ve and +ve

shaalaa.com
  Is there an error in this question or solution?
2016-2017 (March)

APPEARS IN

RELATED QUESTIONS

How much charge is required for the reduction of 1 mol of Zn2+ to Zn?


Write the Nemst equation and explain the terms involved.


Calculate emf of the following cell at 298 K:
Mg(s) | Mg2+(0.1 M) || Cu2+ (0.01) | Cu(s)
[Given Eocell = +2.71 V, 1 F = 96500 C mol–1]


For a general electrochemical reaction of the type:

\[\ce{{a}A + {b}B ⇔ {c}C + {d}D}\]

Nernst equation can be written as:


What is the pH of HCl solution when the hydrogen gas electrode shows a potential of −0.59 V at standard temperature and pressure?


The cell potential for the given cell at 298 K Pt | H2 (g, 1 bar) | H+ (aq) | | Cu2+ (aq) | Cu(s) is 0.31 V. The pH of the acidic solution is found to be 3, whereas the concentration of Cu2+ is 10-x M. The value of x is ______.

[Given: (\[\ce{E_{Cu^{2+}/Cu}}\]) = 0.34 V and `(2.303 " RT")/"F"` = 0.06 V]


Calculate the emf of the following cell at 298 K:

Fe(s) | Fe2+ (0.01 M) | | H+ (1 M) | H2(g) (1 bar) Pt(s)

Given \[\ce{E^0_{cell}}\] = 0.44 V.


Calculate the emf of the following cell at 298 K.

\[\ce{Cu/Cu^{2+}_{(0.025 M)}//Ag^+_{(0.005 M)}/Ag}\]

Given `"E"_("Cu"^(2+)//"Cu")^circ` = 0.34 V, `"E"_("Ag"^+//"Ag")^circ` = 0.80 V

1 Faraday = 96500 C mol -1


Calculate the value of ΔG that can be obtained from the following cell at 298K.

`(Al)/(Al3+) (0.01M) || (Sn^(2+) (0.015M))/(Sn)`

`E^\circ (Al^(3+))/(Al) = -1.66 V;  E^\circ (Sn^(2+))/(Sn) = -0.14 V`


Write the Nernst equation and emf of the following cell at 298 K:

\[\ce{Sn_{(s)} | Sn^{2+} (0.050 M) || H^+ (0.020 M) | H2_{(g)} (1 bar) | Pt_{(s)}}\]


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×